Unit 5 Bonding and Nomenclature 5 1 Nomenclature
Unit 5: Bonding and Nomenclature 5. 1 Nomenclature • • Rules for nomenclature (naming) compounds Formula Writing A. Ionic B. Covalent C. Diatomic 5. 2 Bonding • Ionic and Covalent molecules D. Acids
Unit 5: Terminology List Nomenclature Acids Metals Bases Non-Metals Ionic Combining Capacity (C. C. ) Charges Covalent Bond Polyatomic Ions Roman numerals Diatomics prefixes
5. 1 Nomenclature 2 types: Ionic compounds metals & non-metals Giving/taking electrons Covalent compounds non-metals and non-metals Sharing electrons C
Quick Review: Atomic Symbols e. g. Cl Only capitalize the first letter of a symbol e. g. HCl e. g. Co 2(SO 4)3 vs CO Don´t capitalize the name of chemicals e. g. hydrochloric acid, methane
Chemical Formulas The chemical formula of a substance is a notation that uses atomic symbols with numerical subscripts to convey the relative proportions of atoms of each element in that substance. Consider the formula for aluminum oxide, Al 2 O 3 Compound composed of: O Al O 2 aluminum atoms 3 Oxygen atoms
Part A. Ionic Compounds Metals combined with non-metals Composed of cations and anions Strong attraction between positive (+) and negative (-) charges Ion chart (see Data Booklet)
1. Metals with 1 combining capacity (C. C. ) Metals: • Alkali Metals • Alkaline Earth Metals • Group 3 • Non-Metals: • Halogens • Noble Gases aka: GROUP _______
i) Nomenclature (naming) e. g. Na. Cl = sodium chlor - ide sodium chloride *change the 2 nd elements (non-metal) ending to “-ide” Na = metal; Cl = non-metal (nm) e. g. Li. Br = lithium bromide e. g. Ca. F 2 = calcium fluoride
ii) Formula Writing e. g. aluminum fluoride = e. g. potassium nitride = e. g. calcium oxide = *Reduce Subscripts *Criss-cross method
2. Metals with more than 1 (C. C. )
i) Nomenclature How do you tell the different between the two? ! e. g. Fe. Cl 2 = Iron chloride Fe. Cl 3 = Iron chloride Note: indicate the combining capacity using Roman numerals.
i) Nomenclature Roman numerals: 1. 6. 2. 7. 3. 8. 4. 9. 5. 10.
i) Nomenclature e. g. Pb. O 2 = lead (II) oxide e. g. Cu. I = copper (I) iodide e. g. Cu. I 2 = copper (II) iodide e. g. Co 3 N 2 = cobalt (II) nitride
ii) Writing Formula e. g. tin (II) sulphide = Sn. S e. g. copper (II) phosphide = Cu 3 P 2 e. g. manganese (II) chloride = Mn. Cl 2
LEARNING CHECK - IONIC 1. Sn. S 2 3. Pb. I 4 4. Pb. I 2 5. copper (II) oxide 6. copper (I) oxide 7. iron (II) sulphide 8. chromium (II) iodide
3. Compounds with Polyatomic Ions
i) Nomenclature do not end with “-ide” Use the (polyatomic) Ion Chart (Data Booklet) Examples of polyatomics: Cl. O 3 – = chlorate PO 4 = phosphate NO 3= nitrate OH= hydroxide
i) Nomenclature e. g. Ca(NO 3)2 = e. g. Li. OH = e. g. (NH 4)2 SO 4 = e. g. Cu(OH)2 = e. g. Cu(CO 3) = e. g. Cu. Cl. O =
ii) Writing Formula e. g. lithium sulphate e. g. lithium sulphide Note: do not change the polyatomic ion formula Note: drop brackets for 1 polyatomic ion
ii) Writing Formula e. g. magnesium carbonate =Mg. CO 3 e. g. copper (II) hypochlorite = Cu(Cl. O)2 e. g. chromium (III) hydroxide = Cr(OH)3
LEARNING CHECK - Polyatomics 1. Mn(Mn. O 4)4 2. Mn(SO 4)2 3. copper (I) ethanoate 4. iron (II) sulphate
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